# Problem: How much heat is required to warm 1.50 L of water from 26.0 oC to 100.0 oC? (Assume a density of 1.0 g/mL for the water.)

###### FREE Expert Solution

We’re being asked to determine the amount of heat (Q) needed to raise the temperature of 1.50 L water from 26 ˚C to 100 ˚C

The amount of heat Q is given by:

$\overline{){\mathbf{Q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{∆}}{\mathbf{T}}}$

where m = mass (in grams), c = specific heat, ΔT = change in temperature = final T – initial T.

We’re given the volume of water hence, we need to convert it to its mass by multiplying with the density.

Recall:

$\overline{){\mathbf{density}}{\mathbf{=}}\frac{\mathbf{mass}}{\mathbf{volume}}}$

We’re given the following values:

volume = 1.50 L

density = 1.00 g/mL

c = 4.186 J/g • ˚C (found in books and on the internet)

ΔT = 100 ˚C – 26 ˚C = 74 ˚C

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###### Problem Details

How much heat is required to warm 1.50 L of water from 26.0 oC to 100.0 oC? (Assume a density of 1.0 g/mL for the water.)